Exothermic and endothermic reactions

Question 1

Hard

This question is about the reaction between carbon monoxide ( $CO\text{CO}$ ) and oxygen ( $O2\text{O}_2$ ).

The equation for the reaction is: $2CO(g)+O2(g)→2CO2(g)2\text{CO}(\text{g}) + \text{O}_2(\text{g}) \rightarrow 2\text{CO}_2(\text{g})$

What does $CO2(g)\text{CO}_2(\text{g})$ represent?

[1]

Calculate the volume of oxygen required to react with $cm360\text{ cm}^3$ of carbon monoxide.

[2]

The reaction is exothermic.

Complete the reaction profile shown below:

Reaction profile diagram with the y-axis labeled 'Energy' and the x-axis labeled 'Progress of reaction'. A horizontal line representing the reactants is labeled '2 CO(g) + O2(g)'. From this reactant line, a curve rises to a peak and then begins to curve downwards, but stops before reaching a final horizontal product level.

You should:

complete the profile line
label the activation energy ( $E_a$ )
label the overall energy change ( $ΔH\Delta H$ ).

[3]

The displayed formula equation for the reaction of carbon monoxide with oxygen is: $O=C=O2\ \text{C}\equiv\text{O} \ + \ \text{O}=\text{O} \ \rightarrow \ 2\ \text{O}=\text{C}=\text{O}$

The table below shows some of the bond energies:

Bond	$C≡O\text{C}\equiv\text{O}$	$O=O\text{O}=\text{O}$	$C=O\text{C}=\text{O}$
Bond Energy (kJ/mol)	$1077$	$498$	$X$

In the reaction, the energy released forming new bonds is $kJ/mol544\text{ kJ/mol}$ greater than the energy needed to break existing bonds.

Calculate the bond energy $X$ for the $C=O\text{C}=\text{O}$ bond.

[4]

Exothermic and endothermic reactions

Question 1

Exothermic and endothermic reactions Questions

Exothermic and endothermic reactions

Question 1

Exothermic and endothermic reactions Questions